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18. Which of the following is true? A. When acid is added to pure water, kw, the ion-product constant of water, changes. B. The equilibrium constant of water (keq) is the rate that dissociation of the molecule occurs at room temperature C. The H* (or H³O*) in cells is the same concentration as that of undissociated water D. None of the above E. All of the above

18. Which of the following is true? A. When acid is added to pure water, kw, the ion-product constant of water, changes. B. The equilibrium constant of water (keq) is the rate that dissociation of the molecule occurs at room temperature C. The H* (or H³O*) in cells is the same concentration as that of undissociated water D. None of the above E. All of the above

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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### Multiple Choice Question on Acid-Base Equilibrium #### Question 18: **Which of the following is true?** A. When acid is added to pure water, \( k_w \), the ion-product constant of water, changes. B. The equilibrium constant of water (\( k_{eq} \)) is the rate at which dissociation of the molecule occurs at room temperature. C. The \( H^+ \) (or \( H_3O^+ \)) in cells is the same concentration as that of undissociated water. D. None of the above E. All of the above --- **Explanation:** - **Option A:** When acid is added to pure water, \( k_w \), the ion-product constant of water, generally does change because \( k_w \) is dependent on temperature. - **Option B:** The equilibrium constant (\( k_{eq} \)) of water is not the rate of dissociation but rather a measure of the ratio of products and reactants at equilibrium. - **Option C:** The concentration of \( H^+ \) (or \( H_3O^+ \)) in cells is not the same as that of undissociated water. Cells have regulated pH levels that differ from pure water. - **Option D:** Indicates that none of the provided statements are true. - **Option E:** Indicates that all the provided statements are true. Understanding the fundamental concepts of acid-base equilibrium, such as the ion-product constant of water (\( k_w \)), and equilibrium constants (\( k_{eq} \)), is crucial in the study of chemical reactions in an aqueous solution.
Transcribed Image Text:### Multiple Choice Question on Acid-Base Equilibrium #### Question 18: **Which of the following is true?** A. When acid is added to pure water, \( k_w \), the ion-product constant of water, changes. B. The equilibrium constant of water (\( k_{eq} \)) is the rate at which dissociation of the molecule occurs at room temperature. C. The \( H^+ \) (or \( H_3O^+ \)) in cells is the same concentration as that of undissociated water. D. None of the above E. All of the above --- **Explanation:** - **Option A:** When acid is added to pure water, \( k_w \), the ion-product constant of water, generally does change because \( k_w \) is dependent on temperature. - **Option B:** The equilibrium constant (\( k_{eq} \)) of water is not the rate of dissociation but rather a measure of the ratio of products and reactants at equilibrium. - **Option C:** The concentration of \( H^+ \) (or \( H_3O^+ \)) in cells is not the same as that of undissociated water. Cells have regulated pH levels that differ from pure water. - **Option D:** Indicates that none of the provided statements are true. - **Option E:** Indicates that all the provided statements are true. Understanding the fundamental concepts of acid-base equilibrium, such as the ion-product constant of water (\( k_w \)), and equilibrium constants (\( k_{eq} \)), is crucial in the study of chemical reactions in an aqueous solution.
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